1. G-L’s LAW – Pressure vs. Temperature

2. = P1V1 P2V2 BOYLE’S LAW – Pressure vs. Volume Pressure (kPa)
Volume (mL)

3. = V1 V2 T1 T2 CHARLES’S LAW – Temp vs. Volume Volume (mL)
Temperature (K)

4. Describe the relationship between the temperature of a gas and its pressure.
Solve problems involving temperature-pressure relationships.
Describe some practical applications of Gay-Lussac’s Law.

5. Joseph Gay-Lussac ( )
Determined that temperature and pressure of a gas is a direct relationship (volume and amount of gas are held constant)

6. **As with Charles’ Law, temperature in Kelvin.= P1 P2 T1 T2

7. If a 12. 0 L sample of gas is found to have a pressure of 101
If a 12.0 L sample of gas is found to have a pressure of kPa at 0.0°C, calculate the new pressure at 128°C if the volume is held constant. P1 = P2 T1 T2
0.0°C = 273 K 128°C +273 = 401 K
101.3
149 kPa P2
(401) =
273

8. combined gas law P1 V1 = P2 V2 T1 T2 Boyle’s Law: Pressure α ___1___
volume
Charles’ Law: Volume α temperature
Gay-Lussac’s Law: Pressure α temperature P1 V1 = P2 V2 T1 T2
combined gas law

9. If a gas occupies a volume of 25. 0 L at 25. 0°C and 1
If a gas occupies a volume of 25.0 L at 25.0°C and 1.25 atm, calculate the volume at 128°C and atm. P1 V1 = P2 V2 T1 T2
25°C = 298 K 128°C +273 = 401 K
(1.25) 25 =
56.1 L V2
(401)
298 (0.750)

10. A gas has a volume of 125 L at 325 kPa and 58
A gas has a volume of 125 L at 325 kPa and 58.0°C, calculate the temperature in Celsius to produce a volume of 22.4 L at kPa P1 V1 = P2 V2 T1 T2
58°C = 331 K
18.5 K T2
(101.3)
22.4
(331) =
325 (125)
18.5 K = -254°C

11. A bag contains 145 L of air at the bottom of a lake, at a temperature of 5.20°C and a pressure of 6.00 atm. When the bag is released, it ascends to the surface where the pressure is 1.00 atm and 16.0°C.
Given:
P1 = 6.00 atm V1 = 145L T1 = 5.20°C
P2 = 1.00 atm T2 = 16.0°C
If the maximum volume of the lift bag is 750 L, will the bag burst at the surface?
Find: V2

12. Avogadro’s Hypothesis - any sample of any gas at the same temperature and pressure will contain the same number of particles.

13. Ptotal = P1 + P2 + P3 + P4 … Dalton’s Law of Partial Pressure:
Each gas in a mixture exerts pressure independently.
Total pressure = sum of the pressures of each gas (partial pressures)
Partial pressure depends on the number of gas particles present (moles), the temperature and volume of container.
Ptotal = P1 + P2 + P3 + P4 …

14. 1.0 mol H2
2.0 mol He
3.0 mol gas